SOLVED

61) Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for SO3(g)  ΔH°f (kJ/mol)2 SO2(g) + O2(g) → 2 SO3(g)ΔH°rxn = -198 kJ SO2(g)-297 A) -792 kJ/mol B) -248 kJ/mol C) -495 kJ/mol D) -578 kJ/mol E) -396 kJ/mol 62) Use the information provided to determine ΔH°rxn for the following reaction  ΔH°f (kJ/mol)CH4(g) + 4 Cl2(g) → CCl4(g) + 4 HCl(g)ΔH°rxn = ? CH4(g)-75 CCl4(g)-96 HCl(g)-92 A) -389 kJ B) -113 kJ C) +113 kJ D) -71 kJ E) +79 kJ 63) Use the information provided to determine ΔH°rxn for the following reaction  ΔH°f (kJ/mol)CH4(g) + 3 Cl2(g) → CHCl3(l) + 3 HCl(g)ΔH°rxn = ? CH4(g)-75 CHCl3(l)-134 HCl(g)-92 A) -151 kJ B) -335 kJ C) +662 kJ D) +117 kJ E) -217 kJ 64) Use the information provided to determine ΔH°rxn for the following reaction  ΔH°f (kJ/mol)3 Fe2O3(s) + CO(g) → 2 Fe3O4(s) + CO2(g)ΔH°rxn = ? Fe2O3(s)-824 Fe3O4(s)-1118 CO(g)-111 CO2(g)-394 A) +277 kJ B) -577 kJ C) -47 kJ D) +144 kJ E) -111 kJ 65) How much heat energy is required to raise the temperature of 0.298 mole of water from 35.93°C to 79.84°C? The specific heat capacity of water = 4.18 J/g°C. A) 13.1 J B) 54.7 J C) 985 J D) 2105 J E) 3310 J 66) Which one of the following elements is not in its standard state? A) Br2(g) B) F2(g) C) Hg(l) D) Na(s) E) Cl2(g) 67) A piece of metal weighing 57.3 g is heated to a temperature of 88.0°C and is then immersed in 155 g of water at a temperature of 21.53°C. After equilibration the temperature is 24.72°C. If CH2O = 4.184 J/g°C, what is Cmetal? A) .370 J/g°C B) .164 J/g°C C) 1.00 J/g°C D) 2.11 J/g°C E) .571 J/g°C 68) In a bomb calorimeter, reactions are carried out A) at fixed pressure. B) at fixed volume. C) at fixed temperature. D) with solids only. E) using water as a solvent. 69) For the reaction: NO(g) + 1/2 O2(g) → NO2(g) ΔH°rxn is -114.14 kJ/mol. Calculate ΔH°f of gaseous nitrogen monoxide, given that ΔH°f of NO2(g) is 33.90 kJ/mol. A) 148.0 kJ/mol B) 91.04 kJ/mol C) -114.1 kJ/mol D) 181.9 kJ/mol E) -35.64 kJ/mol 70) Which one of the following statements is not true concerning the equation below? N2(g) + 3 H2(g) → 2 NH3(g)       ΔH°rxn = -459.0 kJ A) The production of 1.00 mole of ammonia is accompanied by the production of 229.5 kJ of heat. B) The complete reaction of 1.00 moles of nitrogen requires 459 kJ of heat. C) The complete reaction of 1.00 moles of hydrogen produces 153 kJ of heat. D) The complete reaction of 0.8278 moles of hydrogen requires 0.2759 moles of nitrogen. E) The reaction is exothermic. 71) Which compound should have the largest lattice energy? A) SrI2 B) CaCl2 C) NaI D) MgO E) KF 72) A sample of NI3 is contained in a piston and cylinder. The samples rapidly decomposes to form nitrogen gas and iodine gas, and releases 3.30 kJ of heat and does 950 J of work. What is ?E? A) -953.3 J B) +953.3 J C) -4250 J D) -946.7 J E) +4250 J 73) A 43.9-g piece of copper (CCu= 0.385 J/g°C) at 135.0°C is plunged into 254 g of water at 39.0°C. Assuming that no heat is lost to the surroundings, what will the final temperature of the system be? A) 100.0°C B) 40.5°C C) 62.5°C D) 87.0°C E) 53.1°C 74) All the following are state functions except A) ?E. B) PV. C) ?H. D) q. E) all of the above are state functions.